- Chapter 7 - Inorganic Chemistry Chemical
Formulas and Chemical Compounds
(textbook pages 218 - 259) Edited by Sydney I and Julia B
Vocabulary
monatomic ion - ion formed from single atom
binary compound - compound composed of two elements
nomenclature - a naming system of binary ionic compounds using the compound's negative and positive ions
oxyanion - a polyatomic ion that contains oxygen
salt - an ionic compound composed of a cation and the anion from an acid
oxidation numbers (oxidation states) - in order to indicate the general distribution of electrons among the bonded atoms in a molecular compoud or a polyatomic ion atoms composing the compound or ion are assigned
formula mass - any molecule, formula unit, or ion is the sum of the average atomic masses of all atoms represented in its formula
percentage composition - the percentage by mass of each element in a compound
empirical formula - consists of the symbols for the elements combined in a compound, with subscripts showing the smallest whole-number mole ration of the different atoms in the compound
~ IONIC - a metal is present ("H" is considered a non-metal)
~ COVALENT- no metal is present
~ HYDRATE - H20 is present
~ ACID - must have "H" at the beginning and be aqueous(aq), meaning it dissolves in water
Naming Covalent Compounds
1.) Tell the number of each element using a prefix.
2.) Change the ending of teh second element to "-ide". *If only one atom of the first element is present, you do NOT use "mono".
Naming Binary Ionic Compounds with a D-Block Metal
Example:
Fe2+Cl22- ~ iron (II) chloride
Fe3+Cl33- ~ iron (III) chloride
Cu2+O2- ~ copper (II) oxide
Cu2+Cl22- ~ copper (II) chloride Cl=1- charge but since there are two, (-1)*2=2-charge
Alternative way... Give the name of the element and if the charge is greater change the ending to "-ic" and if the charge is lesser, change the ending of the name to "-ous"
Latin Name
Element
Charge
ferrum
iron
2+ or 3+
cuprum
copper
1+ or 2+
stannium
tin
2+ or 4+
plumbum
lead
2+ or 4+
Hg
mercury
(mercuric/mercurous)
1+ or 2+
Examples:
Cu2S ~ cupric sulfide or copper (I) sulfide
FeBr2 ~ iron (II) bromide or ferric bromide
SnCl4 ~ stannic chloride or tin (IV) chloride
lead (II) iodine ~ PbI2
cobalt (II) fluoride ~ CoF2
stannous oxide ~ SnO
Naming Ternary (meaning 3 or more) Ionic Compounds
1.) Say the name of the cation.
2.) If the metal is in the d-block, give the charge.
3.) Say the name of the anion.
Examples:
sodium sulfate ~ Na(SO4)
cobalt (II) nitrate ~ CO(NO3)2
iron (II) dichromate or ferrous dichromate ~ FeCr2O7
CuNO3 ~ copper (I) nitrate
(NH4)Cl ~ ammonium chloride
The difference in the prefix and/or suffix happens when oxygens are either dropped or added.
per, -ate = one added
-ate = most common in nature
-ite = one dropped
hypo, -ite = two dropped, least common in nature
- Chapter 7 -
Inorganic Chemistry Chemical
Formulas and Chemical Compounds
(textbook pages 218 - 259)
Edited by Sydney I and Julia B
Vocabulary
~ IONIC - a metal is present ("H" is considered a non-metal)
~ COVALENT- no metal is present
~ HYDRATE - H20 is present
~ ACID - must have "H" at the beginning and be aqueous(aq), meaning it dissolves in water
Naming Covalent Compounds
1.) Tell the number of each element using a prefix.
2.) Change the ending of teh second element to "-ide".
*If only one atom of the first element is present, you do NOT use "mono".
Examples:
P4O10 = tetraphosphorus
NO2 = nitrogen dioxide
H2O = dihydrogen monoxide
N2O4 = dinitrogen tetraoxide
Rules for Naming Binary (meaning two) Ionic Compounds Containing Main Group Metals
1.) Say the name of the cation (HINT: the cation is first).
2.) Say the name of the anion with an "-ide" ending.
Examples:
K2O ~ potassium oxide
CaF2 ~ calcium fluoride
Li2S ~ lithium sulfide
magnesium nitride ~ Mg3N2
sodium phosphide ~ Na3P
calcium oxide ~ CaO
Naming Binary Ionic Compounds with a D-Block Metal
Example:
Fe2+Cl22- ~ iron (II) chloride
Fe3+Cl33- ~ iron (III) chloride
Cu2+O2- ~ copper (II) oxide
Cu2+Cl22- ~ copper (II) chloride
Cl=1- charge but since there are two, (-1)*2=2-charge
Alternative way...
Give the name of the element and if the charge is greater change the ending to "-ic" and if the charge is lesser, change the ending of the name to "-ous"
(mercuric/mercurous)
Examples:
Cu2S ~ cupric sulfide or copper (I) sulfide
FeBr2 ~ iron (II) bromide or ferric bromide
SnCl4 ~ stannic chloride or tin (IV) chloride
lead (II) iodine ~ PbI2
cobalt (II) fluoride ~ CoF2
stannous oxide ~ SnO
Naming Ternary (meaning 3 or more) Ionic Compounds
1.) Say the name of the cation.
2.) If the metal is in the d-block, give the charge.
3.) Say the name of the anion.
Examples:
sodium sulfate ~ Na(SO4)
cobalt (II) nitrate ~ CO(NO3)2
iron (II) dichromate or ferrous dichromate ~ FeCr2O7
CuNO3 ~ copper (I) nitrate
(NH4)Cl ~ ammonium chloride
The difference in the prefix and/or suffix happens when oxygens are either dropped or added.
per, -ate = one added
-ate = most common in nature
-ite = one dropped
hypo, -ite = two dropped, least common in nature
Examples:
ClO4- = perchlorate
ClO3- = chlorate (most common)
ClO2- = chlorite
ClO- = hypochlorite
SO52- = persulfate
SO42- = sulfate (most common)
SO32- = sulfite
SO22- = hyposulfite
Naming Hydrates
Examples:
FeSO4*5H2O = iron (II) sulfate
Ca(NO3)2*2H2O = calcium nitrate dihydrate
Naming Acids
2.) Change anion ending to "-ic".
3.) Say "acid".
2.) Use anion to determine the acid name:
"-ate" goes to "-ic"
"-ite" goes to "-ous"
3.) Say "acid".
H2CO3(aq) ~ carbonic acid
HClO(aq) ~ hypochlorous acid
HI(aq) ~ hydroiodic acid
H2CrO4(aq) ~ chromic acid
H2SO3(aq) ~ sulfurous acid
Polyatomic Ions (also called Radicals)
Practice Problems
Directions: Please write if it is ionic, covalent, an acid, or a hydrate and give its name or formula.
1. Fe2+
2. N2O5
3. sulfuric acid
4. CH3COOH
5. hydrofluoric acid
6. lead (IV) oxide
7. KF
8. phosphorus (III) iodine
9. Hg3(PO4)2
10. HF
Works Cited
Davis, Frey, et al. Modern Chemistry. Orlando: Holt, Rinehart, and Winston, 2006.
http://www.lycos.com/info/acetic
http://chemistry.alanearhart.org/Images/chemist.gif